Question
Wed March 06, 2013 By: Meghana Anil

# The reaction N2 (g)+ O2 (g) (equillibrium arrows)2 NO(g) contributes to air pollution when a fuel is burnt in air at a high temperature.At 1500k quillibruium constant K for it is 1.0x10-5 (no units given).Suppose [N2] =0.8 mol L-1 and [O2]=0.20 mol L-1 before any reaction occurs. Calculate the equillibrium concentraion of the reactants and the product after the mixture has been heated to 1500 k.

Sun March 10, 2013

Let x amount has been decayed from reactant to product then:

N2  +  O2  Ã¢Â†Â” 2NO

T =0  0.8     0.20

T=tequi.  0.8-x   0.2-x  2x

Kc = 1.0 x 10-5

Kc =

1.0 x 10-5 = (2x)2/ [(0.8 - x)(0.2 - x)]

If  x is very small, then

0.8 Ã¢Â€Â“ x Ã¢Â‰Âˆ 0.8

0.2 Ã¢Â€Â“ x Ã¢Â‰Âˆ 0.2

1.0 x 10-5  = (2x)2/ [(0.8 )(0.2)]

16 x 10-6 = 4x2

x= 4 x 10-6

x = 2 x 10-3

Therefore the amount of reactant and product at equilibrium is as follows:

N2 = 0.8 Ã¢Â€Â“ 0.002 = 0.798

O2 = 0.2 Ã¢Â€Â“ 0.002 = 0.198

NO = 2x 2 x 10-3 = 4 x 10-3

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